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Inorganic Chemistry > Solids > Flashcards

Solids Flashcards

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1
Q

Two types of solids

A

Crystalline, amorphous

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2
Q

Solids with a highly regular arrangement of their components. Ex. Diamond, quartz, NaCl

A

Crystalline solids

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3
Q

Solids with considerable disorder in structures. Ex. Plastic, glass, rubber

A

Amorphous

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4
Q

Atoms, ions, or molecules packed in regular geometric arrays are called

A

Lattice

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5
Q

Smallest repeating unit of a lattice

A

Unit cell

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6
Q

Number of nearest neighbor atoms in a lattice

A

Coordination number

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7
Q

Recall summary of unit cells

A

Recall contribution of atoms on each part of a unit cell

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8
Q

Formed when a group MO energy levels with closely spaced energies

A

Band

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9
Q

Valence band: highest energy band

A

Conduction band: partially filled or empty band where electrons can move

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10
Q

Metals are good conductors in lower temp

A

Semiconductors (mettaloids) are good conductors in higher temp

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11
Q

In insulators there is a _____ band gap between valence and conduction bands that prevents the motion of electrons

A

Large

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12
Q

Addition of impurities

A

Doping

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13
Q

Semiconductors whose electrical properties are enhanced by doping

A

Extrinsic semiconductors

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14
Q

____ have small band gap between valence and conduction bands

A

Semiconductors

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15
Q

Elements that exhibit semi-conductive behavior at their pure state are called ____, including Se, Ge, and alpha- Sb

A

Intrinsic semiconductors

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16
Q

The conductivity of intrinsic semiconductors are further enhanced by doping semiconductors with other elements using ____ and ____

A

N-type and P-type dopants

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17
Q

N-type dopants (G15) are capable of doping intrinsic semiconductors because because of their additional _____ relative to the host semiconductor.

A

Free electron.
Note. > valence electron than the element in focus

18
Q

P-type dopants (G13) provide positive ___for increaing the conductance of semiconductors.

A

Holes
Note. < valence electron than the element in focus

19
Q

Mixture of metals and another element

A

Alloy

20
Q

An alloy wherein some of the host metal atoms are replaced by other metal atoms of similar size

A

Substitutional alloys

21
Q

An alloy that is formed when some of the interstices or holes in the closest packed metal structure are occupied by small atoms

A

Interstitial alloy

22
Q

Presence of the interstitial atoms changes the proprties of the host metal

A

Steel is an example of interstitial alloy

23
Q

Solids that are characterized by strong covalent bonding within molecules (IMFA) but relatively weak forces between molecules

A

Molecular solids. They are relatively soft snd have the lowest melting point

24
Q

Solids that are held together by covalent bonds , and have atoms occupying ghe lattice points

A

Network Covalent or Atomic Solids. They have the highest melting point and they’re made up of nonmetals

25
Q

Solids that are high melting substances held together by strong electrostatic forces that exist between oppositely charged ions

A

Ionic solids

26
Q

The structures of most binary ionic solids can be explained by closest packing of spheres. Large anions are packed by either FCC or HCP, while smaller cations fit into holes among the closed packed anions.

A

Packing is done by maximizing the repulsions amon ions with similar charges.

27
Q

Three types of holes in closest packed structures

A

Trigonal, tetrahedral, octahedral ions

28
Q

The stronger the bond that holds the solids together the higher the melting point

A

The smaller size of ion with higher charge the greater the lattice energy

29
Q

___ refers to the change in energy that takes place when separated gaseous ions are packed together to form an ionic solids

A

Lattic energy

30
Q

The process of considering the component reactions that can be imagined as the individual steps in compound formation

A

Born-Haber Cycle

31
Q

Reflects the effect of geometry of lattice on the strength of net coloumbic interaction

A

Madelung constant

32
Q

Recall 7 crystal system
Triclinic
Monoclinic
Orthorhombic
Rhombohedral
Tetragonal
Hexagonal
Cubic

A

CCP- 3 repeating layers
HCP- 2 repeating layers

33
Q

Conduct current at one direction, using pn junction as basis.

A

Diode. Used as rectifiers, voltage regulators, and modulators

34
Q

Formed when semiconductor is exposed to light generating electron-hole pairs, increasing conductivity

A

Photodiode

35
Q

Allows current to be controlled by a small change in potential difference

A

Transistors. Used in amplifiers

36
Q

Solubility of salts in water. In general, the difference in size favors solubility in water. The interaction responsible for lattice enthalpy are replaced with hydration enthalpy.

A

If cation has larger hydration enthalpy than it’s anion partner or vice versa, then the dissolution of salt is exothermic

37
Q

Imperfections of structure or composition contained by all solids

A

Defects

38
Q

Defects that occur in pure substances

A

Intrinsic

39
Q

Defects that stems from the presence of impurities

A

Extrinsic

40
Q

Defects that occur at single site

A

Point defect

41
Q

Defects that occurred in 1, 2 and 3 dimensional. Also gives colors to the gemstones we have.

A

Extended defects

Inorganic Chemistry (12 decks)

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